Lecture Notes: Reactions of Acids with Metals

Introduction

• Topic: How acids react with metals
• Goal: Describe reactions and identify oxidation/reduction for higher tier students
• Key Acids in Chemistry:
  • Hydrochloric Acid (HCl)
  • Sulfuric Acid (H₂SO₄)
  • Nitric Acid (HNO₃)
• Key Fact: All acids contain hydrogen.

Reactivity Series of Metals

• Reactivity Series: Shows how metals are more reactive than hydrogen.
• Displacement Reaction: More reactive metals can displace hydrogen from acids.
• Example Reaction: Sulfuric Acid (H₂SO₄) with Magnesium (Mg)
  • Products: Magnesium Sulfate (MgSO₄) and Hydrogen Gas (H₂)

Products of Acid-Metal Reactions

• General Products: Salt and Hydrogen Gas
• Determining the Type of Salt:
  • Hydrochloric Acid: Produces Chloride salts
  • Sulfuric Acid: Produces Sulfate salts

Reaction Examples

• Magnesium (Mg) Reactions:

  • With Hydrochloric Acid: Produces Magnesium Chloride (MgCl₂) and H₂
  • With Sulfuric Acid: Produces Magnesium Sulfate (MgSO₄) and H₂
  • Reactivity: Rapid reaction due to high reactivity of Mg compared to hydrogen

• Zinc (Zn) Reactions:

  • With Hydrochloric Acid and Sulfuric Acid
  • Reactivity: Rapid reaction; Zn is more reactive than hydrogen

• Iron (Fe) Reactions:

  • With Hydrochloric Acid and Sulfuric Acid
  • Reactivity: Slow reaction; Fe is only slightly more reactive than hydrogen

Exam Notes

• Examiner may ask about reactions of Hydrochloric Acid and Sulfuric Acid with:
  • Magnesium
  • Zinc
  • Iron
• Important: Learn which salts are produced by which acids.

Additional Resources

• Mention of a revision workbook with practice questions available.

Upcoming Topics

• Next video will cover reactions in terms of oxidation and reduction.

These notes provide a summary of how acids react with metals, including product types and reaction dynamics based on metal reactivity.